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2 years ago

Gas occupies 100.0 mL at a pressure of 780 mm Hg. What is the volume of the gas

Chemistry

1 answer:

jolli1 [7]2 years ago

6 0

Answer:

Final volume after applying 880 mmHg pressure = 89.28

Explanation:

Initial volume (V 1)= 100 ml

Initial pressure (P1) =780 mm Hg = 780/780 = 1atm

Final pressure (P2)=880 mm Hg = 880/780 =1.12 atm

Final volume (V2)=?

We know that,

Applying Boyle's law,

P1 V1=P2 V2

1*100=1.12*V2

100=1.12*V2

100/1.12=V2

89.28=V2

V2=89.28 ml

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Entropy change in an internally reversible isothermal process is _______ to the temperature of the system.

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Answer:

Internally reversible is the answer.

Explanation:

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2 years ago

Which two types of consumers are known as “nature’s clean-up crew”? Why are they important?

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3 years ago

Read 2 more answers

On the table below, record your observations before and after the interactions and note if mass was conserved. Describe the chan

lilavasa [31]

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Egg + Heat The egg has a yellow yolk in the middle while there is some type of liquid at the border of the yolk, but it is clear, the heat is hot but transparent The egg turned into a delicious food called an omelet what was yolk staid as a liquid but got a tad harder, but the transparent border around it turned white It was conserved because the eggshell was 4 grams and the fried egg is 41 grams It is a chemical change because it results in the formation of new particles, and the chemical bonds break up and new ones are formed.

Water + Heat The water is a clear liquid, while the heat is very hot but transparent The water turned into a type of oxygen -Water Vapor- If 5 g of water becomes a gas it becomes 5 g of water vapor. The mass of the liquid water is simply transferred into the mass of the newly formed water vapor. There was no chemical reaction because the water vapor can be turned back to water also it just changed from a liquid to a gas and did not change its composition

Zinc + Hydrogen Chloride Zinc: a white/silver metallic solid. Hydrogen chloride (dilute hydroelectric acid) a transparent, colorless liquid with a very low pH (acidic). Zinc "dissolved" in hydrogen chloride, while emitting a colorless gas. The liquid remains a colorless liquid, possibly still having a low pH from the unused acid. The colorless gas collected in a test tube gives a popping sound when ignited with a burning wooden splint, so it is not air embedded in the zinc, nor dissolved in hydroelectric acid. Well although the zinc chloride is 12 grams and not 15 the gas that was released was 3 grams and as we all know 3 + 12 is 15 so you could say that the mass was conserved The production of a new substance (most probably hydrogen) from the reaction of the two reactants. When a few drops of the liquid product are evaporated on a watch glass, a white residue is left. When a few drops of the liquid hydroelectric acid are evaporated on a watch glass, there is no residue. This proves that a new product (hydrogen gas), (white powder, zinc chloride) is produced instead of zinc being physically dissolved in hydroelectric acid.

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3 years ago

7. NH2CO2NH4(s) when heated to 450 K undergoes the following reaction to produce a system which reaches equilibrium: NH2CO2NH4(s

Taya2010 [7]

Answer:

Value of equilibrium constant is 0.0888

Explanation:

Both $NH_{3}$ and $CO_{2}$ are gaseous. Hence equilibrium constant depends upon partial pressures of $NH_{3}$ and $CO_{2}$ .

Initially no $NH_{3}$ and $CO_{2}$ were present.

Hence mole fraction of $NH_{3}$ and $CO_{2}$ at equilibrium can be calculated from coefficient of $NH_{3}$ and $CO_{2}$ in balanced equation.

Mole fraction of $NH_{3}$ = (number of moles of $NH_{3}$ )/(total number of moles of $NH_{3}$ and $CO_{2}$ ) = $\frac{2moles}{(2+1)moles}=\frac{2}{3}$

Mole fraction of $CO_{2}$ = (number of moles of $CO_{2}$ )/(total number of moles of $NH_{3}$ and $CO_{2}$ ) = $\frac{1moles}{(2+1)moles}=\frac{1}{3}$

Let's assume both $CO_{2}$ and $NH_{3}$ behaves ideally.

Therefore partial pressure of $NH_{3}$ , $P_{NH_{3}}= x_{NH_{3}}.P_{total}$ and P_{CO_{2}}= x_{CO_{2}}.P_{total}

Where x represents mole fraction

So, $P_{NH_{3}}=\frac{2}{3}\times 0.843atm=0.562atm$

$P_{CO_{2}}=\frac{1}{3}\times 0.843atm=0.281atm$

So, $K_{p}=P_{NH_{3}}^{2}.P_{CO_{2}}=(0.562)^{2}\times 0.281=0.0888$

4 0

3 years ago

A mixture of H2 and water vapor is present in a closed vessel at 20. 00°C. The total pressure of the system is 755. 0 mmHg. The

MAVERICK [17]

The partial stress of H2 is 737.47 mmHg Let's observe the Ideal Gas Law to find out the whole mols.

We count on that the closed vessel has 1L of volume

P.V=n.R.T
We must convert mmHg to atm. 760 mmHg.
1 atm
755 mmHg (755/760) = 0.993 atm
0.993 m.1L=n.0.082 L.atm/mol.K .
293 K(0.993 atm 1.1L)/(0.082mol.K /L.atm).
293K = n
0.0413mols = n

These are the whole moles. Now we are able to know the moles of water vapor, to discover the molar fraction of it.

P.V=n.R.T
760 mmHg. 1 atm
17.5 mmHg (17.5 mmHg / 760 mmHg)=0.0230 atm
0.0230 m.1L=n.0.082 L.atm/mol.K.293 K(0.0230atm.1L)/(0.082mol.K/L.atm .293K)=n 9.58 × 10 ^ 4 mols = n.
Molar fraction = mols )f gas/general mols.
Molar fraction water vapor =9.58×10^ -four mols / 0.0413 mols
Sum of molar fraction =1
1 - 9.58 × 10 ^ 4 × mols / 0.0413 ×mols = molar fraction H2
0.9767 = molar fraction H2
H2 pressure / Total pressure =molar fraction H2
H2 pressure / 55mmHg = =0.9767 0.9767 = h2 pressure =755 mmHg.
737,47 mmHg.

<h3>What is a mole fraction?</h3>

Mole fraction is a unit of concentration, described to be identical to the variety of moles of an issue divided through the whole variety of moles of a solution. Because it's miles a ratio, mole fraction is a unitless expression.

Thus it is clear that the partial pressure of H2 is 737,47 mmHg.

To learn more about partial pressure refer to the link :

brainly.com/question/19813237

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5 0

2 years ago